A solution of acetic acid, CH 3 COOH, was left on alab shelf with an unknown con

Question

A solution of acetic acid, CH3COOH, was left on alab shelf with an unknown concentration. The pH was found tobe 2.68. What is the concentration of the aceticacid? (Here, find the initial concentration of acetic acid,before ionization, although this concentration may be very similarto the equilibriumconcentration?) Ka=1.8×10-5. Please use steps to help me fully understand how to solve theproblem. Thank you : ) A solution of acetic acid, CH3COOH, was left on alab shelf with an unknown concentration. The pH was found tobe 2.68. What is the concentration of the aceticacid? (Here, find the initial concentration of acetic acid,before ionization, although this concentration may be very similarto the equilibriumconcentration?) Ka=1.8×10-5. Please use steps to help me fully understand how to solve theproblem. Thank you : ) Please use steps to help me fully understand how to solve theproblem. Thank you : )

Explanation / Answer

Use the formula [H+] = (Ka x Concentration ofacid) to solve this problem First, you need to figure out what is the concentration ofH+ present by using pH = -log [H+] pH = -log [H+] 2.68 = -log [H+] [H+] = 0.002089M Then, apply the formula [H+] = (Ka x Concentration of acid) [H+]2 = (Ka x Concentration of acid) 0.0020892 = 1.8 x 10-5 x Concentration ofacid Concentration of acid = 0.243M Hope this helps!

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